The properties of several unknown solids were measured. solid melting point other properties a 1000 ‘c does not conduct electricity

Explanation:A solid compound formed by chemical reaction of a positively charged cation with a negatively charged anion is known as ionic solid. Ionic bonds exist between an ionic solid.When dissolved in water, ionic solids dissociate into ions. Hence, they are able to conduct electricity as electricity is the flow of ions or electrons.A molecular solid is a solid in which molecules are held together by Vander waal forces. They do not conduct electricity as there is no unbalanced charge on the compound.Solids in which atoms of metal are held together by metallic bonds are known as metallic solids. These conduct electricity when present in solid state for bond overlap.A covalent solid is a substance in which atoms are held together by covalent bonds. They do not conduct electricity and have high melting point.Thus, we can conclude the following.A >1000 °C does not conduct electricity : Covalent solidsB 850 °C conducts electricity in the liquid state, but not in the solid state : Ionic solidC 750 °C conducts electricity in the solid state : Metallic solidD 150 °C does not conduct electricity : Molecular solid  

The answer is :Compound A > 1000 ° C does not conduct electricity and is in the form of covalent solidsCompound B = 850 ° C conducts electricity in liquid conditions, but not in solid conditions and the form of ionic solidsCompound C = 750 ° C conducts electricity in solid conditions and the form of metal solidsCompound D = 150 ° C does not conduct electricity and is in the form of a solid moleculeFurther ExplanationElement is a single substance or pure substance that cannot be broken down into simpler substances through chemical reactions. Some chemical scientists have found more than 100 kinds of elements that exist on earth. Based on the periodic system, the elements are grouped into three types, namely metal, semilogene, and non-metal elements.Chemical compounds are pure chemicals that consist of two or several elements that can be broken down into its constituent elements by chemical reactions. For example, dihydrogen monoxide (water, H2O) is a compound consisting of two hydrogen atoms for each oxygen atom. Generally, this comparison must be fixed because of its physical nature, not a comparison made by humans. Therefore, materials such as brass, YBCO superconductors, "aluminum gallium arsenide" semiconductors, or chocolate are considered mixtures or alloys, not compounds. The distinguishing characteristic of compounds is the presence of chemical formulas. The chemical formula provides a ratio of atoms in a substance, and the number of atoms in a single molecule (therefore the chemical formula of ethene is C2H4 and not CH2. The chemical formula does not specify whether the compound is composed of molecules; for example, sodium chloride (table salt, NaCl) is a compound ionic.Type of compoundacidbasesionic compoundsaltthe oxideorganic compoundLearn moredefinition of Chemical compounds definition of Elemen Type of compound DetailsGrade: CollegeSubject: Chemistrykeywords: Chemical compounds

covalentionicmetallicnetwork covalentcovalent bonds are weaker than ionic and create molecular compounds. these have low melting and boiling points. they may/may not be brittle depending upon the salt formed during synthesis. these are usually not polar molecules in that they cannot conduct electricityionic compounds are very strong bonds, it takes a lot of energy to melt and boil these compounds. the bond energies of these bonds are >> bonds found in covalent compounds, these are brittle compounds.metallic bonds are found in metals, of course. these are described as "sea of electrons" because the valence elctrons of each metal atom can freely move between the metal atoms in the crystal. this is what allows for electric conductivity in metals, the easy flow of electrons through the metal.network covalent are covalent bonds. the are different from covalent bonds because they are much stronger bonds. a diamond is made only of C. one sees in other compounds that carbon bonds are covalent and weaker than ionic. in a diamond, the C atoms are in a network of covalent bonds and, as we see everyday, graphite, also only carbon, is so weakly held together that we can rub the tip of a pencil and the C comes off on our hands. another example would be S8. these are covalent yet have a high melting and boiling point. the do not conduct electricity.